How does the pressure of a chemical reaction change when it is filled with gas in a closed container

First of all, in a closed container, fill the reaction gas, you don't have to think about how the pressure changes, because this is the initial state! After that, the change starts according to the initial state! It can also be said that there is no change in the moment of recharge, and the moment of recharge is the initial state!

Explain 2 and 3 first

The meaning of constant capacity and not constant pressure generally refers to the change of the equilibrium system through the change of pressure under the condition of constant temperature and constant volume (volume and temperature always do not change), that is to say, only the change of pressure affects the balance movement.

Constant pressure is not constant volume, which naturally means constant temperature and constant pressure, and only the concentration change caused by the change of volume in the reaction process is considered.

In fact, both of these can be converted into the effect of concentration, which can be understood according to the following explanation.

1. This is generally divided into two situations after equilibration and then filling with the so-called inert gas:

1>. When the constant temperature and capacity, inert gas is filled, because the volume does not change, which will inevitably cause the internal pressure of the container to increase. However, since the volume does not change, and the amount of the reaction gas does not change, the concentration of the reaction gas does not change, so the equilibrium does not move!

It can also be said that although the pressure of the whole vessel increases, the balance does not move because the partial pressure of the reaction gas does not change. See how you understand it.

2>. When the inert gas is filled at constant temperature and pressure, because the pressure remains unchanged, it must only change the volume to ensure the constant pressure! Then the volume will increase, so that the concentration of the reaction gas will decrease, and the equilibrium will move in the direction of the concentration!

All the changes in the analysis process can be regarded as instantaneous changes, just look at the instantaneous changes! As for the images, that's a different story!

There are two scenarios if you fill in gas that does not react.

If it is a constant-capacity container, there is no effect.

If it is a container with constant pressure, it is equivalent to reducing pressure.

The gas pressure can actually be understood as the pressure of the reaction gas, which means that if the gas is irrelevant to the charge, it is enough to analyze the volume change.

Constant capacity or not constant pressure means that the container is fixed, and no matter how the pressure is changed, the volume of the container remains the same.

Constant pressure is not constant volume, which means that the internal pressure is kept constant by changing the volume of the container.

As the pressure increases, the reaction proceeds in the direction of the increase in the volume of the gas.

The pressure is reduced, and the reaction proceeds in the direction of decreasing the volume of the gas.

As long as the coefficient of the gas is compared, it can be judged according to the above principle, but solids and liquids must not be added

The increase in temperature is carried out in the direction of endothermy.

Reducing the temperature is carried out in the direction of heat release.

I said how to score 100 points. There is also a question of add-ons.

Charge the reaction gas, judging by the size of the chemical equation molThe mol number of the generated gas is greater than the mol number of the reaction gas, and the pressure increases. Otherwise, decrease

If it is filled with non-reactive gas. For example, the reaction of conformal gas, constant volume and not constant pressure is carried out in the direction of a small mol numberThe constant voltage is not constant, and the direction should not change.

0 reaction is mainly carried out in a positive direction.

The gas coefficient reaction is generated, and the pressure becomes smaller.

On the contrary, the pressure becomes much greater.

1 becomes larger. 2 Constant volume, due to the reaction proceeding (not equilibrium), the pressure changes.

3 Constant pressure, volume change due to reaction proceeding (non-equilibration).

Constant volume does not mean that the pressure changes after the container is fixed and filled with gas Constant pressure does not mean that the volume of the container can be changed after the gas is flushed, and the pressure is constant through the change of volume.

Summary. The reasons are as follows: any gas pressure is related to the irregular thermal motion of gas molecules, but atmospheric pressure is related to the gravitational pull of the earth in addition to the irregular thermal motion of gas molecules.

Is the pressure of the gas in the container the same as the atmospheric pressure? Explain why.

The first is that it's not exactly the same.

The reasons are as follows: any gas pressure dissipation is related to the irregular thermal movement of gas molecules, but the atmospheric pressure is related to the irregular thermal movement of gas molecules, and is also related to the gravitational pull of the earth.

In addition, the internal pressure of the container is related to the volume of gas inside, and the atmospheric pressure is a fixed value.

The above is my answer, I hope it will be helpful to you.

Ok thanks.

Answer]: C This question examines the safety technology of gas cylinders. Compressed gas: refers to the gas that is completely gaseous after pressurization at -50, including the gas punch body with a critical temperature lower than or equal to -50.

k=[co]·[h2o]/[co2]·[h2]

As the equilibrium constant increases with the increase of temperature, the degree of reaction increases, and according to Shattle's law, it can be seen that the reaction is endothermic.

At this point it is already equilibrium, k = , so the temperature is 830

You have to write the topic clearly.

The pressure change in a confined space is mainly based on whether the gas is consumed or produced in it. Some chemical products can consume oxygen and carbon dioxide in the air, and at the same time, no or less gas is generated, which will reduce the pressure in the container. Many chemical reactions do not consume or produce gases, and the pressure remains the same.

Some chemical reactions produce more gas, which increases the pressure.

Not necessarily, for example: aa+bb=cc+dd

, the pressure does not change.

At C+D, the pressure becomes smaller.

Hope it helps, thanks for adopting.

The so-called airtight container refers to the container that is isolated from the outside world and does not leak air.

There are two types of airtight containers for secondary school:

1. It is an equal-volume airtight container with unchanged volume.

2. It is an isobaric airtight container with constant pressure. (- In the demolition test questions, there are explanations of amusement.) If it is constant temperature and constant volume, the change of pressure before and after the reaction depends on the change of the gas coefficient before and after the reaction, and the pressure remains unchanged if the coefficient before and after the reaction is unchanged, and the gas coefficient and pressure become larger after the reaction, and vice versa.

If the temperature and pressure are constant, the pressure before and after will not change regardless of any reaction.